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Concentrated nitric acid used in the laboratory is 68% nitric acid by mass aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is "1.504 g mL"^(-1)? |
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Answer» Solution :`"68% nitric acid by mass MEANS that"` `"Mass of nitric acid = 68 G,Mass of solution = 100 g"` `"Molar mass of HNO"_(3)="63 g mol"^(-1)` `therefore"68 g HNO"_(3)=(68)/(63)" mole = 1.079 mole,Density of solution = 1.504 g mL"^(-1)` `therefore"VOLUME of solution "=(100)/(1.504)" mL = 66.5 mL = 0.665 L"` `"Molarity of the solution "=("Moles of the solute")/("Volume of solution in L")=(1.079)/(0.0665)M=16.23M` |
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